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Unit Four: Stoichiometry

Total questions: 95

Worksheet time: 3hrs 27mins

Name
Class
Date
1.

What is used to convert between grams and moles?

a)

Avogadro’s number

b)

Molar mass

c)

6.022 x 10^23

d)

Mole ratio

2.

What is used to convert between atoms and moles?

a)

Molar mass

b)

Mole ratio

c)

Periodic table

d)

Avogadro’s number

3.

What is used to convert between moles of two different molecules?

a)

Molar mass

b)

Avogadro’s number

c)

Periodic table

d)

Mole ratio

4.

The Mole Ratio comes from _______ and is used to convert between ________.

a)

Periodic table, grams to moles

b)

Balanced chemical equation, moles of two different molecules

c)

Avogadro’s number, ions to moles

d)

Balanced chemical equation, moles to grams

5.

The molar mass of a compound is found by:

a)

adding the atomic numbers

b)

multiplying by 6.02 X 1023

c)

adding up the masses of all the atoms

d)

multiplying the atomic mass by Avogadro’s number

6.

What is the molar mass of Carbon Tetrachloride (CCl4)?

a)

35.453 g/mol

b)

83.49 g/mol

c)

47.46 g/mol

d)

153.82 g/mol

7.

When the equation below is balanced, what is the mole ratio of Sodium (Na) to Sodium sulfide (Na2S)?


____Na + ____ K2S → ____K + ____ Na2S

a)

1:1

b)

1:2

c)

2:2

d)

2:1

8.

There are 6.022 x 1023 atoms in a mole

a)

True

b)

False

9.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
10.

What is the molar mass of H2O?

a)

18.02 g/mol

b)

33.01 g/mol

c)

17.01 g/mol

11.

Avogadro's number is

a)

used to convert moles to atoms

b)

6.022 x 1023 particles/mole

c)

used to convert molecules to moles

d)

all of the above

12.

The amount of atoms in a mole varies by element

a)

True

b)

False

13.

A mole is a unit

a)

True

b)

False

14.

Balance the following equation:


____Na3PO4 + ____CaCl2 → ____NaCl + ____Ca3(PO4)2

a)

4 : 6 : 12 : 2

b)

2 : 6 : 6 : 1

c)

4 : 3 : 6 : 2

d)

4 : 6 : 4 : 2

15.

What's the "given" in the following problem? How many particles are in 0.250 grams of potassium permanganate (KMnO4)?

a)

0.250 grams KMnO4

b)

particles

c)

KMnO4

d)

0.250

16.

For the balanced reaction below, if 10 moles of NaOH react, how many moles of NaCl are formed?


HCl + NaOH → NaCl + H2O

a)

1 mol NaCl

b)

10 mol NaCl

c)

20 mol NaCl

d)

2 mol NaCl

17.

Particles include

a)

atoms only

b)

molecules only

c)

moles only

d)

molecules and atoms

18.

How many moles of hydrogen (H2) are needed to completely react with two moles of nitrogen (N2)?


____N2 + ____H2 → ____NH3

a)

1 mol H2

b)

6 mol H2

c)

2 mol H2

d)

3 mol H2

19.

Stoichiometry is the:

a)

calculation of amounts of substances in a chemical reaction from the balanced equation

b)

calculation of the mass of substances in a chemical reaction from the chemical equation

c)

calculation of the number of particles in a physical reaction from the balanced equation

d)

bane of my existence

20.

What is the most important piece of information necessary to perform a stoichiometric calculation?

a)

Number of moles

b)

Number of particles

c)

Liters of gas

d)

Mass of reactants

e)

A balanced chemical equation

21.

Using stoichiometry, you can determine which of the following? (more than one answer may apply)

a)

mass of products given the mass of reactants

b)

mass of a salt produced by the reaction between two volumes of gas

c)

number of reactant molecules needed to produce 150 grams of product

d)

how much water can be made by burning methane

22.

A certain automobile contains 4 tires, 2 headlights, 1 steering wheel, and 6 spark plugs. How many of each part will be required to build 17 of these cars?

a)

66 tires, 32 headlights, 15 steering wheels, 102 spark plugs

b)

72 tires, 48 headlights, 17 steering wheels, 96 spark plugs

c)

68 tires, 34 headlights, 17 steering wheels, 102 spark plugs

d)

68 tires, 32 headlights, 17 steering wheels, 102 spark plugs

23.

The reaction of sodium with water produces sodium hydroxide and hydrogen gas: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) How many moles of water are needed to react with 0.89 moles of sodium?

a)

0.445

b)

0.89

c)

1.01

d)

1.78

24.

The reaction of aluminum metal with an aqueous solution of silver nitrate produces aqueous aluminum nitrate and solid silver metal. What is the balanced chemical equation describing this reaction?

a)

Al (s) + 3 AgNO3 (aq) → Al(NO3)3 (aq) + 3 Ag (s)

b)

Al + 3 AgNO3 → Al(NO3)3 + 3 Ag

c)

Al (aq) + AgNO3 (s) → Al(NO3)2 (aq) + 3 Ag (g)

d)

Al(s) + SiNi8 (aq) → AlNi8 (aq) + Si (s)

25.

The reagent which determines how much product will be made is the _______ reagent

a)

deficient

b)

rate-limiting

c)

limiting

d)

restricted

26.

The excess reagent is the material that is

a)

used up in the reaction

b)

left over

c)

brings stoichiometric balance

d)

makes extra product

27.

True/False: All reactions need an excess reagent.

a)

True

b)

False

28.

To identify the excess reagent, all data must be in ______ quantities

a)

molal

b)

molecular

c)

mass

d)

molar

29.

True/False: A balanced equation allows us to determine the excess reagent.

a)

True

b)

False

30.

The theoretical yield is

a)

the amount you hope to get

b)

the maximum amount that can be formed from the given amounts of reactants

c)

the amount you need for the next reaction

d)

the actual amount you obtain in the reaction

31.

17. Actual yield is

a)

the amount you obtain in the reaction

b)

the amount you want to obtain in the reaction

c)

the amount of product using excess reagent

d)

the amount of product before purification

32.

In the reaction A+B→C+D, 7.2 moles A form 5.4 moles C. The mole ratio A:C is

a)

2:1

b)

4:2

c)

2:3

d)

4:3

33.

How many moles of I2 are produced if 4.7 moles Br2 are reacted with excess FeI3?

a)

4.7

b)

9.4

c)

14.1

d)

18.8

34.

What mass of zinc oxide will be formed from 20.0 g of zinc?

a)

10.5 g

b)

19.8 g

c)

24.9 g

d)

32.3 g

35.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
36.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
37.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
38.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 3 moles of Fe2O3?
a)
6 moles Fe
b)
4 moles Fe
c)
2 moles Fe
d)
1 moles Fe
39.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
40.

In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen (aluminum is asked for, oxygen is given)?

a)

10/6

b)

3/4

c)

4/3

d)

2/3

41.

In the reaction 2 H2 + O2 → 2 H2O what is the mole ratio of oxygen to water

a)

1/2

b)

2/1

c)

3/4

d)

4/3

42.

What is the molar mass of table salt (NaCl)?

a)

116.89 g/mol

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

43.

What is the molar mass of NaOH?

a)

40.00 g/mol

b)

38.99 g/mol

c)

23.99 g/mol

d)

57.00 g/mol

44.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
45.
What is the percent yield of the following reaction if 145g of P2O5 reacts with 40 grams of water, but you only collected 112 grams of phosphoric acid? 3 H2O + P2O5 -> 2H3PO4
a)
80%
b)
85%
c)
77%
d)
58%
46.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
47.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
48.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
49.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
50.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
51.
What is the empirical formula for the following:
Pb5Cr5O20
a)
Pb2Cr2O10
b)
PbCr2O7
c)
Pb9Cr4O2
d)
PbCrO4
52.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements so that you can give the correct name of the compound formed.

a)

Sulfur monoxide

b)

Sulfur dioxide

c)

Sulfur trioxide

d)

Sulfur tetroxide

53.

Calculate the percent water in strontium chloride hexahydrate

a)

6.76%

b)

59.45%

c)

68.21%

d)

40.55%

54.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
55.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
56.

Na2CO3 · 10H2O is known as sodium carbonate ______

a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
57.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
58.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)

contains water in the compound

d)
repels water from the compound
59.

How do you calculate the percent by mass of an element in a compound? 

a)

Add up the mass of protons and neutrons, then divide by two.

b)

Divide the mass of the element by the total mass of the compound and multiply by 100.

c)

Add up the atomic masses of the elements, then divide by the number of the elements.

d)

Find the relative mass of any atom by adding the number of protons to the number of neutrons, then dividing by that total number.

60.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
61.

Determine the formula of CuSO4·?H2O hydrate given the following data:

Test Tube = 23.56 g

Test Tube + Hydrate = 26.06 g

Test Tube + Anhydrate = 25.16 g

a)

CuSO4·H2O

b)

CuSO4·2H2O

c)

CuSO4·4H2O

d)

CuSO4·5H2O

62.

Name the following ionic compound: MgSO4 • 7H2O

a)

magnesium sulfide hexahydrate

b)

magnesium sulfite heptahydrate

c)

magnesium sulfate heptahydrate

d)

magnesium sulfide heptahydrate

63.

A 5.018 gram sample of a certain hydrate of magnesium sulfate, MgSO4 • xH2O, is heated until all the water is driven off. The resulting anhydrous compound weighs 2.449 grams. What is the formula of the hydrate?

a)

MgSO4 • 9H2O

b)

MgSO4 • 8H2O

c)

MgSO4 • 7H2O

d)

MgSO4 • 6H2O

64.

Find the percent composition of Cu2S?

a)

Cu= 67.987%; S= 32.013%

b)

Cu= 79.854%: S= 20.145%

c)

Cu= 35.946%; S= 64.054%

d)

Cu= 39.925%; S= 20.151%

65.

Dried or without water

a)

anhydrate/anhydride

b)

hydrate

c)

grapes

66.

A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the waters of hydration. The mass after heating was reduced to 7.58 g. Calculate the percent water by mass in the original hydrate.

a)

7.58 %

b)

8.09%

c)

48.37%

d)

51.63%

67.

A 3.11 g sample of ZnSO4 ⋅ 7H2O is heated to dryness. Determine the mass of anhydrous salt remaining after all the water has been driven off.

a)

3.11 g

b)

1.75 g

c)

1.36 g

d)

0.562 g

68.
How do we name a hydrate?
a)
Add "water" to the end of the chemical name
b)
Use a prefix and add hydrate
c)
Do nothing, it does not change
69.

What is the best method for removing water from a hydrated compound?

a)

freezing

b)

filtration

c)

distillation

d)

heating

70.

Calculate the percent water by mass in cobalt(II) chloride dihydrate, CoCl₂•2H₂O.

a)

36.0%

b)

78.3%

c)

21.7%

d)

10.9%

e)

13.9%

71.

How many step will it take for me to go from moles given to moles unknown?

a)

1

b)

2

c)

3

d)

4

72.

4 Al + 3 O2 –> 2 Al2O3 How much aluminum would be needed to completely react with 45 grams of O2?

a)

1.05 moles

b)

3.75 moles

c)

0.875 grams

d)

1.875 moles

73.

How many grams of H2O will be formed when 32.0 g H2 is allowed to react with 16.0 g O2 according to

2 H2 + O2 → 2 H2O

a)

9.00 g

b)

16.0 g

c)

18.0 g

d)

32.0 g

e)

36.0 g

74.

When 2.00 g of H2 reacts with 32.0 g of O2 in an explosion, the final gas mixture will contain:

a)

H2, H2O, and O2

b)

H2 and H2O only

c)

O2 and H2O only

d)

H2 and O2 only

e)

H2O only

75.

The reaction of 7.8 g benzene, C6H6, with excess HNO3 resulted in 0.90 g of H2O. What is the percentage yield? Molar Mass (g/mol):

C6H6=78 HNO3=63 C6H5NO2=123 H2O=18

C6H6 + HNO3 → C6H5NO2 + H2O

a)

100%

b)

90%

c)

50%

d)

12%

e)

2%

76.

How many grams of nitric acid, HNO3, can be prepared from the reaction of 138 g of NO2 with 54.0 g H2O according to the equation below?

3NO2 + H2O → 2HNO3 + NO

a)

92

b)

108

c)

126

d)

189

e)

279

77.

Calculate the mass of hydrogen formed when 27 g of aluminum reacts with excess hydrochloric acid according to the balanced equation below. 2Al + 6HCl → 2 AlCl3 + 3 H2

a)

1.5 g

b)

2.0 g

c)

3.0 g

d)

6.0 g

e)

12 g

78.

Identify the limiting reactant when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.


Mg + 2HCl --> MgCl2 + H2

a)

Mg

b)

H2

c)

MgCl2

d)

HCl

79.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
80.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
81.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
82.
What does percent yield indicate?
a)
The amount of product we should get
b)
The efficiency of the lab
c)
The amount of product we actually got
d)
nothing
83.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
84.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
85.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
86.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron can be made from 6 moles H2 and excess Fe2O3?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

87.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
88.
Lead nitrate can be decomposed by heating.  What is the % yield of the decomposition reaction if 7.4g Pb(NO3)2 are heated to give 4.1 g PbO?
2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)
a)
82%
b)
44%
c)
56%
d)
67%
89.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
90.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
91.

Identify the limiting and excess reactants in the reaction shown.

a)

N2 is limiting and H2 is excess. 

b)

H2 is limiting and N2 is excess. 

c)

NH3 is both limiting and excess.

d)

There is no limiting reactant. 

92.

Aluminum reacts with hydrochloric acid according to:

2Al + 6HCl → 2AlCl3 +3H2

If 4.0 g of Al react with 10.0 g of HCl, which reactant is in excess?

a)

Al

b)

HCl

93.

C3​H8​ + 5O2​ → 3CO2 ​+ 4H2​O

A sample contains 5.0 g of propane and 20.0 g of oxygen. Which reactant is in excess?

a)

Propane

b)

Oxygen

94.

2H2​ + O2​ → 2H2​O

You mix 3.0 g of H₂ with 16.0 g of O₂.
After the reaction goes to completion, how many grams of the excess reactant remain?

a)

2.0 g

b)

4.0 g

c)

8.0 g

d)

1.0 g

95.

2Na + Cl2​→ 2NaCl

If 12 g of Na react with 15 g of Cl₂, what mass of the excess reactant is left over after the reaction?

a)

2.3 g

b)

5.6 g

c)

7.2 g

d)

9.4 g

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